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Calculate the maximum ionic character possible in a bond between two atoms in the periodic table according to Hanny Smith equation. [Electronegativeity of Li=1.0, Na=0.9, K=0.8, Rb=0.8, Cs=0.7, Fr=0.7]
1.  $~90\%$
2.  $~97\%$
3.  $~80\%$
4.  $~75\%$

Choose the correct order from the following:
1.  ${\mathrm{N}}_2\mathrm{O}<{\mathrm{N}}_2{\mathrm{O}}_3<\mathrm{NO}$ ; Acidic character
2.  $\mathrm{MgO}>{\mathrm{Al}}_2{\mathrm{O}}_3>{\mathrm{SiO}}_2$ ; Basic character
3.  ${\mathrm{Fe}}^{3+}<{\mathrm{Fe}}^{2+}<{\mathrm{Mn}}^{2+}$ ; Ionic radius order
4.  $\mathrm{Sc}>\mathrm{La}>\mathrm{Y}$ ; Ionisation energy order

Statement-1 : Fluorine (F) act as stronger oxidizing agent than oxygen (O).
Statement-2 :$\left|∆{\mathrm{H}}_{\mathrm{e}.\mathrm{g}.\mathrm{e}}\right|$ of Fluorine (F) is higher than oxygen (O).
1.  Statement-1 is true, statement-2 is true and statement-2 is correct explanation for statement-1.
2.  Statement-1 is true, statement-2 is true and statement-2 is not the correct explanation for statement-1.
3.  Statement-1 is true, statement-2 is false.
4.  Statement-1 is false, statement-2 is true.

Choose the correct statement(s).
1.  Lattice energy $\mathrm{\alpha }\frac{1}{{\mathrm{r}}^2}$. [where r is the interionic distance]
2.  Lattice energy $\mathrm{\alpha } {\mathrm{q}}_1{\mathrm{q}}_2$. [where ${\mathrm{q}}_1 \& {\mathrm{q}}_2$ are the charges of co-ions]
3.  Ionic mobility of the ions in aqueous state $\mathrm{\alpha }\frac{1}{\mathrm{radius} \mathrm{of} \mathrm{ions} \mathrm{in} \mathrm{gaseous} \mathrm{state}}$
4.  Heat of formation of a compound depends on the number of steps involved in its formation reaction.

Statement-1: Glycerol is more viscous than methanol.
Statement-2: This is due to intramolecular H-bonding.
1.  Statement-1 is true, statement-2 is true and statement-2 is correct explanation for statement-1.
2.  Statement-1 is true, statement-2 is true and statement-2 is not the correct explanation for statement-1.
3.  Statement-1 is true, statement-2 is false.
4.  Statement-1 is false, statement-2 is true.

${\mathrm{AsF}}_5$ molecule is trigonal bipyramidal. The hybrid orbitals used by As-atoms for bonding are
1.  ${\mathrm{d}}_{{\mathrm{x}}^2-{\mathrm{y}}^2}, {\mathrm{d}}_{{\mathrm{z}}^2}, \mathrm{s}, {\mathrm{p}}_{\mathrm{x}}, {\mathrm{p}}_{\mathrm{y}}$
2.  ${\mathrm{d}}_{\mathrm{xy}}, \mathrm{s}, {\mathrm{p}}_{\mathrm{x}}, {\mathrm{p}}_{\mathrm{y}}, {\mathrm{p}}_{\mathrm{z}}$
3.  $\mathrm{s}, {\mathrm{p}}_{\mathrm{x}}, {\mathrm{p}}_{\mathrm{y}}, {\mathrm{p}}_{\mathrm{z}}, {\mathrm{d}}_{{\mathrm{z}}^2}$
4.  ${\mathrm{d}}_{{\mathrm{x}}^2-{\mathrm{y}}^2}, \mathrm{s}, {\mathrm{p}}_{\mathrm{x}}, {\mathrm{p}}_{\mathrm{y}}, {\mathrm{p}}_{\mathrm{z}}$

Choose the incorrect statement among the following.
1.  $\mathrm{HF}$ is the most volatile acid among $\mathrm{HX}$.
2.  ${\mathrm{Na}}_2{\mathrm{O}}_2$ is having ionic and covalent type of bonds.
3.  ${\mathrm{CH}}_3{\mathrm{CO}}_2\mathrm{Na}$ is having identical $\mathrm{C}-\mathrm{O}$ bond lengths while it is not true for ${\mathrm{CH}}_3{\mathrm{CO}}_2\mathrm{H}$.
4.  p-p overlap is more stronger compared to s-s overlap in axial type of bond formation.

Find out the molecule species which is not electron deficient.
1.  ${\mathrm{AlCl}}_3$
2.  ${\mathrm{BeH}}_2$
3.  ${{\mathrm{BH}}_4}^{-}$
4.  ${\mathrm{BF}}_3$

Choose the correct $1^{\mathrm{st}}$ ionisation potential order of the given elements.
1.  $\mathrm{B}<\mathrm{Be}<\mathrm{N}<\mathrm{O}$
2.  $\mathrm{Be}<\mathrm{B}<\mathrm{N}<\mathrm{O}$
3.  $\mathrm{N}>\mathrm{Be}>\mathrm{O}>\mathrm{B}$
4.  $\mathrm{N}>\mathrm{O}>\mathrm{Be}>\mathrm{B}$

Choose the incorrect statement.
1.  Electronegativity of $\mathrm{Cl}$ is less than $\mathrm{F}$.
2.  Electron affinity of $\mathrm{Cl}$ is greater than $\mathrm{F}$.
3.  Bond energy of $\mathrm{\sigma }$-bond is greater than $\mathrm{\pi }$ bond.
4.  The net dipole moment direction of ${\mathrm{NF}}_3$ is toward $\mathrm{l}.\mathrm{p}.$ of N-atom.

If y-axis is the approaching axis between two atoms, then which of the set of orbitals cannot form the $\mathrm{\pi }$ bond between two atoms in general.
1.  ${\mathrm{P}}_{\mathrm{y}}-{\mathrm{P}}_{\mathrm{z}}$
2.  ${\mathrm{P}}_{\mathrm{x}}-{\mathrm{P}}_z$
3.  ${\mathrm{P}}_{\mathrm{x}}-{\mathrm{P}}_{\mathrm{y}}$
4.  None of these

In which of the following molecule the intramolecular hydrogen bonding is not existing.
1.  chloral hydrate
2.  0-chlorophenol
3.  choral
4.  salicylic acid

The number of $\mathrm{P}-\mathrm{O}-\mathrm{P}$ linkages in ${\mathrm{P}}_4{\mathrm{O}}_{10}$ and ${\mathrm{P}}_4{\mathrm{O}}_6$ are respectively -
1.  6,6 
2.  6, 8
3.  8, 6
4.  8, 8

The state of hybridisation of 'B' atoms in borax $\left({\mathrm{Na}}_2{\mathrm{B}}_4{\mathrm{O}}_7 · 10{\mathrm{H}}_2\mathrm{O}\right)$ is
1.  All sp² hybridised
2.  Three sp² and one sp³ hybridised
3.  One sp² and three sp³ hybridised
4.  Two sp² and two sp³ hybridised

Which of the following forces does not contribute to the van der Waal's forces of attraction.
1.  Dipole-dipole interaction
2.  Dipole-induced dipole interaction
3.  Instantaneous dipole induced dipole interaction
4.  ELectrostatic forces of attraction releasing the energy 72 kJ/mole

For the molecule ${\mathrm{MA}}_2{\mathrm{L}}_{\mathrm{n}}$ (where A is number of single bonded surrounding atoms, L indicates lone pair and 'n' is the number of lone pair and M is the central atom of 's' or 'p' block element) the possible range of 'n' is
1.  '1' to '4'
2.  zero to '4'
3.  '1' to '3'
4.  '0' to '3'

The total number of $\mathrm{\pi }$-bond electrons in the following structure is
                   
1.  4
2.  8
3.  12
4.  16

Carbon suboxide $\left({\mathrm{C}}_3{\mathrm{O}}_2\right)$ has
1.  Linear structure
2.  Bent structure
3.  Trigonal structure
4.  Distorted tetrahedral structure

Which of the following gas is least polarizable?
1.  He
2.  Ne
3.  Kr
4.  Xe

Which of the following is correct order of dipole moment of the following?
         
1.  I  > II > III
2.  I = II = III
3.  III > II > I
4.  I > III > II

${\mathrm{PCl}}_5$ is highly unstable and in solid state it exists as into ${\left[{\mathrm{PCl}}_4\right]}^{+} \mathrm{and} {\left[{\mathrm{PCl}}_6\right]}^{-}$ ions.
The geometry of ${\left[{\mathrm{PCl}}_6\right]}^{-}$ is
1.  octahedral
2.  tetrahedral
3.  square pyramidal
4.  square planar

In an octahedral structure, the pair of d orbitals involved in ${\mathrm{d}}^2{\mathrm{sp}}^3$-hybridisation is
1.  ${\mathrm{d}}_{{\mathrm{x}}^2-{\mathrm{y}}^2}, {\mathrm{d}}_{{\mathrm{z}}^2}$
2.  ${\mathrm{d}}_{\mathrm{xy}}, {\mathrm{d}}_{{\mathrm{x}}^2-{\mathrm{y}}^2}$
3.  ${\mathrm{d}}_{{\mathrm{z}}^2}, {\mathrm{d}}_{\mathrm{xz}}$
4.  ${\mathrm{d}}_{\mathrm{xy}}, {\mathrm{d}}_{\mathrm{yz}}$

In ${\mathrm{PO}}_4^{3-}$ ion, the formal charge on each oxygen atom and P-O bond order respectively are :
1.  -0.75, 0.6
2.  -0.75, 1.0
3.  -0.75, 1.25
4.  -3.1, 1.25

The correct order of increasing bond angles in t
he following species is
1.  ${\mathrm{Cl}}_2\mathrm{O} < {\mathrm{ClO}}_2 < {\mathrm{ClO}}_2^{-}$
2.  ${\mathrm{ClO}}_2 < {\mathrm{Cl}}_2\mathrm{O} < {\mathrm{ClO}}_2^{-}$
3.  ${\mathrm{Cl}}_2\mathrm{O} < {\mathrm{ClO}}_2^{-} < {\mathrm{ClO}}_2$
4.  ${\mathrm{ClO}}_2^{-} < {\mathrm{Cl}}_2\mathrm{O} <{\mathrm{ClO}}_2$

Which of the following compounds has the lowest melting point?
1.  ${\mathrm{CaBr}}_2$
2.  ${\mathrm{Cal}}_2$
3.  ${\mathrm{CaF}}_2$
4.  ${\mathrm{CaCl}}_2$